問題一覧
1
A homogeneous mixture composed of two or more substances.
2
Water
3
Solvent
4
Solute
5
Solute-solute and solvent-solvent interactions
6
The ions separate and interact with water molecules.
7
The maximum quantity of solute that can dissolve in a specific amount of solvent at a particular temperature.
8
A solution containing more solute than can normally dissolve at a given temperature.
9
Unsaturated
10
Solute-solvent interaction
11
Unsaturated
12
Supersaturated
13
Saturated
14
Increasing temperature increases solubility.
15
Henry's Law
16
Like dissolves like
17
Nonpolar solute with nonpolar solvent
18
Salt in water, Sugar in water
19
Partial pressure
20
Solid in solid
21
Increasing partial pressure
22
Gas in gas solution
23
Agitation (stirring)
24
Nitrate (NO3-), Group 1 ions (Li+, Na+, K+, Rb+, Cs+), Ammonium (NH4+), Acetates
25
Lead(II) sulfate (PbSO4)
26
Ba2+, Ca2+, Sr2+, Pb2+, Hg2+, Ag+
27
Group 1 ions, NH4+
28
Nitrates, Acetates
29
Pb2+, Ag+, Hg2+
30
Hydroxides are insoluble except with Group 1, NH4+, Ba2+, Ca2+, and Sr2+
31
It is always soluble.
32
Calcium phosphate (Ca3(PO4)2)
33
They help predict whether a substance will dissolve in water., They are essential for writing net ionic equations., They aid in preparing chemical solutions.
34
Moles of solute per liter of solution
35
Molarity (mol/L), Percent concentration (%), Molality (mol/kg), Normality (eq/L), Parts per million (ppm)
36
To ensure accurate calculations and meaningful comparisons
37
(grams of solute / grams of solution) × 100
38
Moles of solute per kilogram of solvent
39
Adding more solvent to decrease concentration while keeping the amount of solute unchanged.
40
C1V1 = C2V2
41
Measure a volume V1 from a stock solution with known concentration C1.
42
It remains unchanged.
43
To prepare solutions from a more concentrated stock solution.
44
5.10%
45
5.0 N
46
(Volume of solute/Volume of solution) × 100%
47
60 mL
48
The molar mass of NH3
49
sour
50
red
51
hydrogen gas
52
OH⁻ ions
53
hydronium ion (H₃O⁺)
54
It only includes substances that contain OH⁻ ions as bases.
55
A proton donor
56
Conjugate base
57
A substance that can act as either an acid or a base
58
Bicarbonate (HCO₃⁻)
59
It accepts an electron pair.
60
Bronsted-Lowry acid: proton donor
61
Lewis definition
62
Water and a salt
63
Lewis acid
64
It completely ionizes in water
65
HI, HCl, H2SO4, HClO3, HNO3
66
An equilibrium is established between the un-ionized species and its conjugate, Both reactants and products are present in the solution
67
(C2H5)NH, NH3, NH2NH2, NHOH, C5H5N
68
It is a strong acid or base
69
It completely ionizes in water
70
LiOH, NaOH, Mg(OH)2, Ca(OH)2, Sr(OH)2
71
An acid that can donate more than one acidic hydrogen
72
Stepwise, with each hydrogen ion being released in a separate equilibrium step
73
Two
74
Three
75
Auto-ionization
76
1.0 x 10^-14
77
They resist changes in pH when small amounts of acid or base are added.
78
The Henderson-Hasselbalch equation
79
OH⁻ ions react with HF to form F⁻ and water, minimizing the increase in pH.
80
The mathematical definition of pH in terms of hydronium ion concentration
81
The concentration of the conjugate base
82
F⁻ ions neutralize H⁺ ions, forming more HF and preventing a significant drop in pH.
83
Titrant
84
It changes color to signal the end point of the titration.
85
Equivalence Point
86
The substance whose concentration is being determined.
87
The point at which the indicator changes color, signaling completion of the reaction.
88
Indicator
89
Its concentration.
90
To determine the concentration of an unknown solution.
91
Catalyst
92
The calculated concentration of analyte will be inaccurate.
93
Compounds that change color when they undergo protonation or deprotonation
94
They change color at a specific pH range to approximate the equivalence point
95
It changes color
96
The endpoint of the titration
97
M = amount of substance (mol) / volume (L)
98
It turns pale pink at the endpoint
99
Ba(OH)₂ + 2HCl → BaCl₂ + 2H₂O
100
Yellow to blue
問題一覧
1
A homogeneous mixture composed of two or more substances.
2
Water
3
Solvent
4
Solute
5
Solute-solute and solvent-solvent interactions
6
The ions separate and interact with water molecules.
7
The maximum quantity of solute that can dissolve in a specific amount of solvent at a particular temperature.
8
A solution containing more solute than can normally dissolve at a given temperature.
9
Unsaturated
10
Solute-solvent interaction
11
Unsaturated
12
Supersaturated
13
Saturated
14
Increasing temperature increases solubility.
15
Henry's Law
16
Like dissolves like
17
Nonpolar solute with nonpolar solvent
18
Salt in water, Sugar in water
19
Partial pressure
20
Solid in solid
21
Increasing partial pressure
22
Gas in gas solution
23
Agitation (stirring)
24
Nitrate (NO3-), Group 1 ions (Li+, Na+, K+, Rb+, Cs+), Ammonium (NH4+), Acetates
25
Lead(II) sulfate (PbSO4)
26
Ba2+, Ca2+, Sr2+, Pb2+, Hg2+, Ag+
27
Group 1 ions, NH4+
28
Nitrates, Acetates
29
Pb2+, Ag+, Hg2+
30
Hydroxides are insoluble except with Group 1, NH4+, Ba2+, Ca2+, and Sr2+
31
It is always soluble.
32
Calcium phosphate (Ca3(PO4)2)
33
They help predict whether a substance will dissolve in water., They are essential for writing net ionic equations., They aid in preparing chemical solutions.
34
Moles of solute per liter of solution
35
Molarity (mol/L), Percent concentration (%), Molality (mol/kg), Normality (eq/L), Parts per million (ppm)
36
To ensure accurate calculations and meaningful comparisons
37
(grams of solute / grams of solution) × 100
38
Moles of solute per kilogram of solvent
39
Adding more solvent to decrease concentration while keeping the amount of solute unchanged.
40
C1V1 = C2V2
41
Measure a volume V1 from a stock solution with known concentration C1.
42
It remains unchanged.
43
To prepare solutions from a more concentrated stock solution.
44
5.10%
45
5.0 N
46
(Volume of solute/Volume of solution) × 100%
47
60 mL
48
The molar mass of NH3
49
sour
50
red
51
hydrogen gas
52
OH⁻ ions
53
hydronium ion (H₃O⁺)
54
It only includes substances that contain OH⁻ ions as bases.
55
A proton donor
56
Conjugate base
57
A substance that can act as either an acid or a base
58
Bicarbonate (HCO₃⁻)
59
It accepts an electron pair.
60
Bronsted-Lowry acid: proton donor
61
Lewis definition
62
Water and a salt
63
Lewis acid
64
It completely ionizes in water
65
HI, HCl, H2SO4, HClO3, HNO3
66
An equilibrium is established between the un-ionized species and its conjugate, Both reactants and products are present in the solution
67
(C2H5)NH, NH3, NH2NH2, NHOH, C5H5N
68
It is a strong acid or base
69
It completely ionizes in water
70
LiOH, NaOH, Mg(OH)2, Ca(OH)2, Sr(OH)2
71
An acid that can donate more than one acidic hydrogen
72
Stepwise, with each hydrogen ion being released in a separate equilibrium step
73
Two
74
Three
75
Auto-ionization
76
1.0 x 10^-14
77
They resist changes in pH when small amounts of acid or base are added.
78
The Henderson-Hasselbalch equation
79
OH⁻ ions react with HF to form F⁻ and water, minimizing the increase in pH.
80
The mathematical definition of pH in terms of hydronium ion concentration
81
The concentration of the conjugate base
82
F⁻ ions neutralize H⁺ ions, forming more HF and preventing a significant drop in pH.
83
Titrant
84
It changes color to signal the end point of the titration.
85
Equivalence Point
86
The substance whose concentration is being determined.
87
The point at which the indicator changes color, signaling completion of the reaction.
88
Indicator
89
Its concentration.
90
To determine the concentration of an unknown solution.
91
Catalyst
92
The calculated concentration of analyte will be inaccurate.
93
Compounds that change color when they undergo protonation or deprotonation
94
They change color at a specific pH range to approximate the equivalence point
95
It changes color
96
The endpoint of the titration
97
M = amount of substance (mol) / volume (L)
98
It turns pale pink at the endpoint
99
Ba(OH)₂ + 2HCl → BaCl₂ + 2H₂O
100
Yellow to blue